Kinetics, Maxwell-Boltzmann Distribution, and Reaction Rates

Flashcards covering key vocabulary, chemical kinetics concepts, Maxwell-Boltzmann distributions, factors affecting reaction rates, and relative reaction rates from the lecture transcripts.

Maxwell-Boltzmann distribution

A graph showing the distribution of kinetic energy ($KE$) of particles at a certain temperature.

Activation energy ($E_a$)

The threshold kinetic energy required for collisions to react; particles with $KE < E_a$ cannot react, while particles with $KE \neq E_a$ or $KE \neq E_a$ (effective collisions) can react.

Catalyst

A factor that increases the reaction rate by orders of magnitude by enabling a greater fraction of collisions to be effective; it is the only variable that changes activation energy ($E_a$).

Temperature relationship to rate

Temperature ($T$) is exponentially proportional to reaction rate, where for every $10\,^\circ\text{C}$ increase in temperature, the reaction rate doubles.

Surface Area

A variable directly proportional to reaction rate because increasing it increases the number of exposed particles and the collisions between reactants.

Rate Law

A function that calculates the instantaneous rate of a reaction with a certain concentration of reactants for a general equation $aA + bB \rightarrow \text{products}$.

Rate of disappearance of $N_2(g)$

The rate given as $30\,\text{atm/min}$ in the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$.

Initial pressures ($P_i$) in example reaction

For the reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$, the initial pressures are $P_i(N_2) = 1.0\,\text{atm}$, $P_i(H_2) = 3.0\,\text{atm}$, and $P_i(NH_3) = 0\,\text{atm}$.